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Solved: (a) The nitric oxide molecule, NO, readily loses
Chapter , Problem 9.82a(choose chapter or problem)
(a) The nitric oxide molecule, NO, readily loses one electron to form the NO+ ion. Which of the following is the best explanation of why this happens: (i) Oxygen is more electronegative than nitrogen, (ii) The highest energy electron in NO lies in a p2*p molecular orbital, or (iii) The p2*p MO in NO is completely filled.
Questions & Answers
QUESTION:
(a) The nitric oxide molecule, NO, readily loses one electron to form the NO+ ion. Which of the following is the best explanation of why this happens: (i) Oxygen is more electronegative than nitrogen, (ii) The highest energy electron in NO lies in a p2*p molecular orbital, or (iii) The p2*p MO in NO is completely filled.
ANSWER:Problem 9.82a +(a) The nitric oxide molecule, NO, readily loses one electron to form the NO ion. Whichof the following is the best explanation of why this happens: (i) Oxygen is moreelectronegative than nitrogen, (ii) The highest energy electron in NO lies in a p2 *molecular orbital, or (iii) The p2 * MO in NO is completely filled. (b) Predict the order of + -the NO bond strengths in NO, NO , and NO , and describe the magnetic properties of each,.(c) With what neutral homonuclear diatomic molecules are the NO and NO ions isoelectronic(same number of electrons) Step-by-step solution Step 1 of 4 ^Nitric oxide NO is the simplest stable oxide of nitrogen and is the simplest odd electronmolecule known so far. The Lewis structure of NO is given below.This structure does not satisfy the octet rule and also there is no evidence that the moleculeexists as a dimer. The unpaired electron does not reside on the nitrogen instead it is sharedbetween oxygen and nitrogen.